Module 6 Portage Learning Chemistry
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Amorphous solids - ansparticles are arranged in a random fashion
Colligative properties - ansphysical properties of solvents that are dependent on the
concentration of the solute present and the identity of the solvent but not on the identity
of the solute. They include vapor pressure, freezing point and boiling point
Colloids - ansheterogeneous mixtures which appear to homogeneous one-phase
mixtures but are actually composed of particles too small to be seen with the naked eye
Condensation - ansprocess of gas being converted to liquid
Critical point - ansthe temperature above which a substance cannot exist in the liquid
phase
Critical pressure - ansthe lowest pressure required for the substance to exist as a liquid
at the critical point
Crystalline solids - ansparticles are arranged in one of several different orderly,
repeating, geometric patterns
Describe/define the Tyndall effect - ansColloids can be distinguished from solutions by
use of a beam of light which is scattered by colloids but passes un-scattered through a
solution, a result known as the Tyndall effect
Differentiate between a crystal lattice and a unit cell - ansA crystal lattice is the orderly,
repeating geometric pattern in which the particles of a crystalline solid are arranged.
The unit cell is the smallest section of the crystal lattice having that arrangement of
particles
Differentiate between evaporation and vaporization - ansVaporization is the conversion
of liquid particles to vapor at the boiling point temperature of the material. The process
of liquid converting to vapor molecules can also take place in a very limited manner at
temperatures lower than the boiling point and is called evaporation
Electrolytes - ansionic or very polar compounds which dissolve to form solutions of ions
which conduct an electric current
Explain how and why the presence of a solute affects the boiling point of a solvent -
ansThe presence of a solute raises the boiling point of a solvent by lowering the vapor
pressure of the solvent. With this lower vapor pressure, more heat (a higher boiling
point) is required to raise the vapor pressure to atmospheric pressure
Explain how and why the presence of a solute affects the freezing point of a solvent -
ansThe presence of a solute lowers the freezing point of a solvent by forcing solvent
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molecules away from the growing solid crystal. In order for the solvent molecules to
reach the crystal and add themselves to the freezing solid, they must be slowed down to
a lower kinetic energy by lowering the temperature
Explain how and why the presence of a solute affects the vapor pressure of a solvent -
ansThe presence of a solute lowers the vapor pressure of a solvent because some of
the solute particles occupy the space near the surface of the liquid replacing some of
the solvent particles thereby decreasing the rate at which solvent particles can enter the
vapor
Explain the difference in the properties of graphite and diamond which are both pure
carbon - ansIn graphite the atoms are arranged in planes which can slide relative to one
another making graphite a good solid lubricant. In diamond the atoms are arranged in
tetrahedrons which are tightly bonded together making carbon the hardest substance
known.
Explain water's concave meniscus in terms of cohesive and adhesive forces -
ansCohesive forces are the attractions between particles of the same type, such as the
bonds between water molecules whereas adhesive forces are attractions between a
particle of one type and particles of a different type, such as the bonds between water
molecule and those of its glass container. These cohesive and adhesive forces combine
to cause liquids to form a meniscus (curved surface) in a glass tube. A liquid with strong
cohesive forces, such as water, tries to roll itself into a ball to minimize surface tension,
but water is also attracted to the walls of any tube by adhesive forces, causing the water
to form a concave meniscus.
Explain why sugar can be made to dissolve more quickly by grinding it to a fine crystal -
ansGrinding sugar to a fine crystal increases the surface area of the crystal and this
makes it dissolve more quickly because solute particles dissolve by leaving the surface
of their bulk structure which is in contact with the solvent
Explain why the vapor pressure of a liquid increases with increasing temperature -
ansWater molecules in the liquid state freely vibrate and rotate. As the temperature
rises, the vibrations and rotations become intense enough to overcome the forces that
keep the molecules together. The molecules begin to undergo translational motion
allowing the molecules to convert to the vapor state and these exert a pressure above
the still-existing liquid molecules called the vapor pressure of the substance. Higher
temperature = greater conversion to vapor = higher vapor pressure
Fluids - anssubstances like liquids and gases which have no fixed shape and so they
flow
Ionization - ansthe splitting of molecules to form ions
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List and describe the two components of a solution - ansThe minor component of a
solution which is being dissolved is called the solute while the major component doing
the dissolving is called the solvent.
Molality - ansthe number of moles of solute present per kilogram of solvent
Molarity - ansthe number of moles of solute present per liter of solution
Nonelectrolytes - anscompounds which dissolve to form solutions of molecules which
do not conduct an electric current
Phase - ansany state of matter such as solid, liquid or gas
Strong electrolytes - anssolutes that ionize completely
Sublimation - ansthe conversion of a solid directly to the gas state
Surface tension - ansthe force that causes a liquid which is in contact with a gas like air
to assume a shape that has the least amount of surface area causing the surface to act
like a thin elastic sheet
Triple point - ansthe temperature and pressure at which the solid, liquid and gas phases
can coexist
Vapor pressure - anspressure exerted by vapor molecules above a liquid
Weak electrolytes - anssolutes that only partially ionize
What rule is used to predict the solubility of materials? - ansThe "like dissolves like" rule
is used to predict the solubility of materials with polar solvents only dissolving polar (and
ionic) substances and nonpolar solvents only dissolving nonpolar substances.
Why are liquids the least common state of matter? - ansthey can exist only within a
relatively narrow range of temperatures and pressures
Why does a bottle of soda pop "fizz" when it is opened? - ansWhen a bottle of soda pop
is opened, the pressure above the solution decreases and some of the carbon dioxide
bubbles off since a lower pressure allows the gas molecules in the solution to escape
Why does a phase change occur at one temperature rather than over a temperature
range? - ansDuring a phase change, the temperature of the material remains constant
as all of the energy being added is being used to overcome forces of attraction between
the particles and separate them so the temperature does not rise. Over any other
portions of the temperature range, when a material is heated, the temperature of the
latest 2024 |Already graded A+
Amorphous solids - ansparticles are arranged in a random fashion
Colligative properties - ansphysical properties of solvents that are dependent on the
concentration of the solute present and the identity of the solvent but not on the identity
of the solute. They include vapor pressure, freezing point and boiling point
Colloids - ansheterogeneous mixtures which appear to homogeneous one-phase
mixtures but are actually composed of particles too small to be seen with the naked eye
Condensation - ansprocess of gas being converted to liquid
Critical point - ansthe temperature above which a substance cannot exist in the liquid
phase
Critical pressure - ansthe lowest pressure required for the substance to exist as a liquid
at the critical point
Crystalline solids - ansparticles are arranged in one of several different orderly,
repeating, geometric patterns
Describe/define the Tyndall effect - ansColloids can be distinguished from solutions by
use of a beam of light which is scattered by colloids but passes un-scattered through a
solution, a result known as the Tyndall effect
Differentiate between a crystal lattice and a unit cell - ansA crystal lattice is the orderly,
repeating geometric pattern in which the particles of a crystalline solid are arranged.
The unit cell is the smallest section of the crystal lattice having that arrangement of
particles
Differentiate between evaporation and vaporization - ansVaporization is the conversion
of liquid particles to vapor at the boiling point temperature of the material. The process
of liquid converting to vapor molecules can also take place in a very limited manner at
temperatures lower than the boiling point and is called evaporation
Electrolytes - ansionic or very polar compounds which dissolve to form solutions of ions
which conduct an electric current
Explain how and why the presence of a solute affects the boiling point of a solvent -
ansThe presence of a solute raises the boiling point of a solvent by lowering the vapor
pressure of the solvent. With this lower vapor pressure, more heat (a higher boiling
point) is required to raise the vapor pressure to atmospheric pressure
Explain how and why the presence of a solute affects the freezing point of a solvent -
ansThe presence of a solute lowers the freezing point of a solvent by forcing solvent
,Module 6 Portage Learning Chemistry
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molecules away from the growing solid crystal. In order for the solvent molecules to
reach the crystal and add themselves to the freezing solid, they must be slowed down to
a lower kinetic energy by lowering the temperature
Explain how and why the presence of a solute affects the vapor pressure of a solvent -
ansThe presence of a solute lowers the vapor pressure of a solvent because some of
the solute particles occupy the space near the surface of the liquid replacing some of
the solvent particles thereby decreasing the rate at which solvent particles can enter the
vapor
Explain the difference in the properties of graphite and diamond which are both pure
carbon - ansIn graphite the atoms are arranged in planes which can slide relative to one
another making graphite a good solid lubricant. In diamond the atoms are arranged in
tetrahedrons which are tightly bonded together making carbon the hardest substance
known.
Explain water's concave meniscus in terms of cohesive and adhesive forces -
ansCohesive forces are the attractions between particles of the same type, such as the
bonds between water molecules whereas adhesive forces are attractions between a
particle of one type and particles of a different type, such as the bonds between water
molecule and those of its glass container. These cohesive and adhesive forces combine
to cause liquids to form a meniscus (curved surface) in a glass tube. A liquid with strong
cohesive forces, such as water, tries to roll itself into a ball to minimize surface tension,
but water is also attracted to the walls of any tube by adhesive forces, causing the water
to form a concave meniscus.
Explain why sugar can be made to dissolve more quickly by grinding it to a fine crystal -
ansGrinding sugar to a fine crystal increases the surface area of the crystal and this
makes it dissolve more quickly because solute particles dissolve by leaving the surface
of their bulk structure which is in contact with the solvent
Explain why the vapor pressure of a liquid increases with increasing temperature -
ansWater molecules in the liquid state freely vibrate and rotate. As the temperature
rises, the vibrations and rotations become intense enough to overcome the forces that
keep the molecules together. The molecules begin to undergo translational motion
allowing the molecules to convert to the vapor state and these exert a pressure above
the still-existing liquid molecules called the vapor pressure of the substance. Higher
temperature = greater conversion to vapor = higher vapor pressure
Fluids - anssubstances like liquids and gases which have no fixed shape and so they
flow
Ionization - ansthe splitting of molecules to form ions
, Module 6 Portage Learning Chemistry
latest 2024 |Already graded A+
List and describe the two components of a solution - ansThe minor component of a
solution which is being dissolved is called the solute while the major component doing
the dissolving is called the solvent.
Molality - ansthe number of moles of solute present per kilogram of solvent
Molarity - ansthe number of moles of solute present per liter of solution
Nonelectrolytes - anscompounds which dissolve to form solutions of molecules which
do not conduct an electric current
Phase - ansany state of matter such as solid, liquid or gas
Strong electrolytes - anssolutes that ionize completely
Sublimation - ansthe conversion of a solid directly to the gas state
Surface tension - ansthe force that causes a liquid which is in contact with a gas like air
to assume a shape that has the least amount of surface area causing the surface to act
like a thin elastic sheet
Triple point - ansthe temperature and pressure at which the solid, liquid and gas phases
can coexist
Vapor pressure - anspressure exerted by vapor molecules above a liquid
Weak electrolytes - anssolutes that only partially ionize
What rule is used to predict the solubility of materials? - ansThe "like dissolves like" rule
is used to predict the solubility of materials with polar solvents only dissolving polar (and
ionic) substances and nonpolar solvents only dissolving nonpolar substances.
Why are liquids the least common state of matter? - ansthey can exist only within a
relatively narrow range of temperatures and pressures
Why does a bottle of soda pop "fizz" when it is opened? - ansWhen a bottle of soda pop
is opened, the pressure above the solution decreases and some of the carbon dioxide
bubbles off since a lower pressure allows the gas molecules in the solution to escape
Why does a phase change occur at one temperature rather than over a temperature
range? - ansDuring a phase change, the temperature of the material remains constant
as all of the energy being added is being used to overcome forces of attraction between
the particles and separate them so the temperature does not rise. Over any other
portions of the temperature range, when a material is heated, the temperature of the
